Course Objective(s):
This course will enable the students to –
Course Outcomes (COs):
Course Outcomes
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On completion of this course, the students will be able to; CO45: describe the concept of thermal equilibrium and laws of thermodynamics. CO46: apply the first law of thermodynamics for closed systems to calculate thermodynamic properties. CO47: describe Hess's law of constant heat summation and Kirchoff's relations to calculate enthalpy change. CO48: calculate entropy for various processes and transformation. CO49: explain the concept of partial molar properties for open system. CO50: apply various laws of thermodynamics to explain the behavior of chemical equilibrium. |
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Importance and scope, system and surroundings, type of systems (isolated, closed and open), extensive and intensive properties, steady state and equilibrium state, concept of thermodynamic equilibrium, zeroth-law of thermodynamics, state of a system, state functions and path functions, partial derivatives and cyclic rule.
Concept of heat(q), work(W), internal energy(U), enthalpy(H) and first law of thermodynamics, calculation of q, W, U and H for reversible and irreversible processes and free expansion of gases (ideal and van der Waals) under isothermal and adiabatic conditions, graphical explanation of work done during expansion and compression of an ideal gas.
Heat changes at constant volume and constant pressure, relation between CP and CV using ideal gas and van der Waals’ equations, Joule's experiment and its consequence, explanation of term (δU/δV)T, Joule-Thomson experiment and its consequences, Joule-Thomson coefficient for a van der Waals’ gas, inversion temperature.
Heat changes during physicochemical processes at constant pressure/volume. Heat of reaction- enthalpy of formation, enthalpy of combustion, enthalpy of neutralization, enthalpy of ionization, enthalpy of solution, enthalpy of phase transition, Hess's law of constant heat summation and applications, bond enthalpy, Kirchoff's relations.
Second law of thermodynamics- need for the second law, concept of heat reservoirs and heat engines, Kelvin, Planck and Clausius statements, Carnot cycle, Carnot theorem.
Physical concept of entropy, variation of entropy with temperature, pressure and volume, entropy change for various processes, entropy change during the isothermal mixing of ideal gases.
Third law of thermodynamics, Nernst Heat Theorem, concept of residual entropy, auxiliary state functions (G and A) and their variation with T, P and V, criteria for spontaneity and equilibrium.
Thermodynamic relations- Maxwell's relations, thermodynamic equation of state, Gibbs-Helmholtz equation.
Open system, chemical potential, partial molar quantities, variation of chemical potential with temperature and pressure, Gibbs-Duhem equation, chemical potential for the mixing of ideal gases, determination of partial molar quantities, fugacity and fugacity coefficient.
Chemical Equilibrium: Criteria of thermodynamic equilibrium, degree of advancement of reaction, Equilibrium constant and relationship between KP, KC and Kx , standard Gibbs free energy change in a chemical reaction: Van't Hoff's reaction isotherm, van't Hoff's reaction isobar and isochore, chemical equilibria in ideal gases, thermodynamic derivation of relation between Gibbs free energy of a reaction and reaction quotient, equilibrium constants and their dependence on temperature, pressure and concentration, Le Chatelier’s principle (quantitative treatment), free energy of mixing and spontaneity, equilibrium between ideal gases and a pure condensed phase.
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